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19 July, 17:33

A chemist designs a galvanic cell that uses these two half-reactions:

half-reaction standard reduction potential

MnO4⁻ (aq) + 8H⁺ (aq) + 5e⁻ → Mn (aq) ²⁺ + 4H2O (l) E⁰red = + 1.51V

Fe³⁺ (aq) + e⁻ → Fe²⁺ (aq) E⁰red = + 0.771V

Answer the following questions about this cell.

(a) Write a balanced equation for the half-reaction that happens at the cathode.

(b) Write a balanced equation for the half-reaction that that happens at the anode.

(c) Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

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  1. 19 July, 18:04
    0
    MnO4⁻ (aq) + 8H⁺ (aq) + 5Fe³⁺ (aq) →Mn (aq) ²⁺ + 4H2O (l) + 5Fe²⁺ (aq)

    Explanation:

    a)

    MnO4⁻ (aq) + 8H⁺ (aq) + 5e⁻ → Mn (aq) ²⁺ + 4H2O (l)

    b)

    5Fe³⁺ (aq) + 5e⁻ → 5Fe²⁺ (aq)

    c)

    MnO4⁻ (aq) + 8H⁺ (aq) + 5Fe³⁺ (aq) →Mn (aq) ²⁺ + 4H2O (l) + 5Fe²⁺ (aq)
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